🧪 GCSE Chemistry Revision Newsletter - Diamond

Part 1 - Keywords:

• Diamond

• Giant Covalent Structure

• Covalent Bonds

• Carbon Atoms

• Tetrahedral Network

• Hardness

• Melting Point

• Non-Conductive

Part 2 - Key Facts:

• Diamond is a giant covalent structure where each carbon atom is bonded to four others.

• The carbon atoms form a tetrahedral network, creating a very strong and rigid structure.

• Diamond has no free electrons, meaning it does not conduct electricity.

• Diamond’s rigid structure makes it extremely hard, which is useful for cutting tools.

• Diamond has a very high melting point, similar to silica, due to the strong covalent bonds.

• Uses of diamond include diamond-tipped glass cutters, oil rig drills, and other cutting tools.

Part 3 - Quick Quiz:

1. What kind of structure does diamond have?

   • A) Ionic

   • B) Metallic

   • C) Giant Covalent

2. How many carbon atoms is each carbon atom in diamond bonded to?

   • A) 2

   • B) 4

   • C) 6

3. Why is diamond useful for cutting tools?

   • A) It has free electrons

   • B) It is very soft

   • C) It is extremely hard

Answers:

1. C

2. B

3. C

Part 4 - Going Further:

Question: Explain why diamond does not conduct electricity but has a very high melting point.

Answer: Diamond does not conduct electricity because it has no free electrons; all the electrons are involved in covalent bonds between the carbon atoms. However, diamond has a very high melting point because of its giant covalent structure. The strong covalent bonds between the carbon atoms require a lot of energy to break, giving diamond its high melting point and making it one of the hardest natural materials.

Part 5 - Revision Tips:

When revising giant covalent structures like diamond, focus on understanding the arrangement of atoms and the type of bonding. Remember that covalent bonds in a tetrahedral network lead to the hardness and high melting points.

Part 6 - More Help:

Here are two useful webpages and one YouTube video to help with revising the chemistry topic of diamond:

1. BBC Bitesize - Diamond and Graphite
   This page explains the structure and properties of diamond, including why it’s so hard, why it doesn’t conduct electricity, and its uses in tools and jewellery. It also compares diamond with graphite, another form of carbon.

2. Shalom Education - Diamond Revision
   This webpage offers a detailed overview of diamond's covalent structure, explaining how each carbon atom bonds to four others, forming a strong and durable structure. It covers properties such as hardness, high melting point, and non-conductivity​

3. YouTube - Diamond and Graphite (GCSE Chemistry) | SnapRevise
   This video explains the differences between diamond and graphite, focusing on their structure, bonding, and key properties that make them unique. It’s a great visual aid for revising the topic.

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Stay tuned for the next issue where we’ll cover another interesting giant covalent structure: graphite!

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